Question

Read the following table and chose the appropriate option

Rate equation	Units of K
I) rate $=$ k[A]	a) mol lit${}^{-1}$ sec ${}^{-1}$
II) rate $=$ k[A][B]	b) mol${}^{-2}$ lit${}^2$ sec ${}^{-1}$
III) rate $=$ k[A][B]${}^2$	c) sec ${}^{-1}$
IV) rate $=$ k	d) lit mol${}^{-1}$ sec ${}^{-1}$

• A. I - d, II - c, III - a, IV - b
• B. I - c, II - d, III - b, IV - a
• C. I - a, II - b, III - c, IV - d
• D. I - b, II - a, III - d, IV - c

Answer 1

The correct option is B I - c, II - d, III - b, IV - a

Units of k $=mol{e}^{1-n}li{t}^{n-1}se{c}^{-1}$ , where n is the order of reaction.

For option A, its first order reaction. Rate constant $=se{c}^{-1}$

For option B, its second order reaction. Rate constant $=mol{e}^{-1}litse{c}^{-1}$

For option C, its third order reaction. Rate constant $=mol{e}^{-2}li{t}^{2}se{c}^{-1}$

For option D, its zero order reaction. rate constant $=mole/litse{c}^{-1}$

Hence, the correct option is $\text{B}$